Textbook Question
Using only the periodic table as your guide, select the most electronegative atom in each of the following sets: (a) Se, Te, Br, I; (b) Be, Mg, C, Si (c) Al, Si, P, S (d) Zn, Ge, Ga, As.
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Ch.8 - Basic Concepts of Chemical Bonding
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 8, Problem 37b
(b) How many bonding electrons are in the structure?
Verified step by step guidance1
Step 1: Understand the concept of bonding electrons. Bonding electrons are the electrons that are shared between atoms in a molecule, forming covalent bonds.
Step 2: Identify the molecule or compound in question. Without this information, we cannot proceed further.
Step 3: Draw the Lewis structure of the molecule. This will help visualize the arrangement of atoms and the distribution of electrons.
Step 4: Count the number of covalent bonds in the Lewis structure. Each covalent bond consists of two bonding electrons.
Step 5: Multiply the number of covalent bonds by two to find the total number of bonding electrons in the structure.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Bonding Electrons
Bonding electrons are the electrons that are involved in the formation of chemical bonds between atoms. These electrons are typically found in pairs and are shared between atoms in covalent bonds or transferred in ionic bonds. Understanding the number of bonding electrons is crucial for determining the stability and reactivity of a molecule.
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03:37
Bond Angles and Electron Groups
Lewis Structures
Lewis structures are diagrams that represent the arrangement of atoms and the distribution of electrons in a molecule. They illustrate how bonding and lone pairs of electrons are organized, allowing chemists to visualize the connectivity and electron sharing between atoms. Analyzing a Lewis structure helps identify the number of bonding electrons present.
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04:28Lewis Dot Structures: Ions
Valence Electrons
Valence electrons are the outermost electrons of an atom that are involved in chemical bonding. The number of valence electrons determines how an atom interacts with others, influencing its ability to form bonds. Knowing the valence electron count is essential for constructing Lewis structures and understanding the bonding characteristics of a molecule.
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Related Practice
Textbook Question
Using Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms, showing valence-shell electrons. e. How many bonding pairs of electrons are in the SiCl4 molecule?
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Textbook Question
Place the following pairs of elements in order from smallest to largest difference in electronegativity: K and F, S and O, Br and I, Ca and Se, Li and Cl.
Textbook Question
Using Lewis symbols and Lewis structures, diagram the formation of PF3 from P and F atoms, showing valence-shell electrons. (a) How many valence electrons does P have initially? (c) How many valence electrons surround the P in the PF3 molecule? (d) How many valence electrons surround each P in the PF3 molecule?
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Textbook Question
Which of the following statements about electronegativity is or are true? i. The alkali metals are the family with the largest electronegativity values. ii. The numerical values for electronegativity have no units. iii. Electronegativity is the ability of an atom in a molecule to attract electron density toward itself.
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